Here we will provide you the 50+ MCQ Questions of Thermodynamics for NEET-UG. Thermodynamics is the chapter 6 in Class XI or Class 11 Chemistry NCERT Unit Thermodynamics NEET (conducted by NTA) is based on the NCERT book.
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Thermodynamics NEET MCQ
Which of the following thermodynamic quantities is always negative for a spontaneous process at constant temperature and pressure?
a) Gibbs free energy
b) Enthalpy
c) Entropy
d) Internal energy
The change in entropy of a system undergoing a reversible process between two equilibrium states is given by:
a) ΔS = Q/T
b) ΔS = Qrev/T
c) ΔS = dS/dt
d) ΔS = dU/dT
The standard enthalpy of formation of NH3(g) at 298 K is -46.1 kJ/mol. The standard Gibbs free energy change for the formation of NH3(g) under standard conditions is:
a) -46.1 kJ/mol
b) -16.6 kJ/mol
c) +46.1 kJ/mol
d) +16.6 kJ/mol
The standard Gibbs free energy change for the reaction A(g) + B(g) → C(g) is -50 kJ/mol at 298 K. If the equilibrium constant for the reaction at the same temperature is 10^3, the standard Gibbs free energy change for the reverse reaction is:
a) -50 kJ/mol
b) 50 kJ/mol
c) 24.6 kJ/mol
d) -24.6 kJ/mol
The maximum amount of work that can be obtained from a system at constant temperature and pressure is equal to:
a) ΔG
b) ΔH
c) TΔS
d) -TΔS
Which of the following thermodynamic quantities is not a state function?
a) Internal energy
b) Enthalpy
c) Entropy
d) Heat
For an ideal gas, the internal energy is a function of:
a) Temperature only
b) Pressure only
c) Volume only
d) Temperature and volume
A system absorbs 500 J of heat and performs 250 J of work. What is the change in internal energy of the system?
a) +250 J
b) -250 J
c) +750 J
d) -750 J
For a spontaneous process, which of the following statements is true?
a) ΔH > 0 and ΔS > 0
b) ΔH < 0 and ΔS > 0
c) ΔH > 0 and ΔS < 0
d) ΔH < 0 and ΔS < 0
The standard enthalpy of combustion of methane gas (CH4) at 298 K is -890.3 kJ/mol. What is the standard enthalpy of formation of methane gas at 298 K?
a) -74.9 kJ/mol
b) -74.6 kJ/mol
c) -74.4 kJ/mol
d) -74.1 kJ/mol
Which of the following thermodynamic quantities is an extensive property?
a) Enthalpy
b) Entropy
c) Internal energy
d) Heat capacity
The change in enthalpy of a system undergoing a process at constant pressure is equal to:
a) ΔH = Q
b) ΔH = Q – PΔV
c) ΔH = ΔU + PΔV
d) ΔH = ΔU – PΔV
The entropy of a perfect crystal at absolute zero is:
a) Zero
b) Positive
c) Negative
d) Undefined
The change in Gibbs free energy of a system is given by:
a) ΔG = ΔH – TΔS
b) ΔG = ΔH + TΔS
c) ΔG = ΔU + PΔV
d) ΔG = ΔU – PΔV
For a spontaneous process, which of the following statements is true?
a) ΔG > 0 and ΔS > 0
b) ΔG < 0 and ΔS > 0
c) ΔG > 0 and ΔS < 0
d) ΔG < 0 and ΔS < 0
The work done in an isothermal reversible expansion of an ideal gas is given by:
a) W = nRTln(V2/V1)
b) W = nRTln(P2/P1)
c) W = -nRTln(V2/V1)
d) W = -nRTln(P2/P1)
The standard Gibbs free energy change for the reaction A(g) + B(g) → 2C(g) is +50 kJ/mol at 298 K. If the partial pressure of C is doubled at the same temperature, the standard Gibbs free energy change for the reaction:
a) Remains the same
b) Doubles
c) Halves
d) Becomes zero
The standard entropy of vaporization of water at 100°C is 109.0 J/mol K. What is the standard enthalpy of vaporization of water at 100°C?
a) 40.7 kJ/mol
b) 39.6 kJ/mol
c) 38.7 kJ/mol
d) 37.8 kJ/mol
The enthalpy change for the reaction H2(g) + 1/2O2(g) → H2O(l) is -285.8 kJ/mol. What is the enthalpy change for the reverse reaction?
a) +285.8 kJ/mol
b) -285.8 kJ/mol
c) -571.6 kJ/mol
d) +571.6 kJ/mol
The heat capacity of a substance is given by:
a) C = ΔH/ΔT
b) C = ΔU/ΔT
c) C = ΔS/ΔT
d) C = Q/ΔT
The Clausius-Clapeyron equation relates:
a) The change in enthalpy with temperature
b) The change in entropy with temperature
c) The change in pressure with temperature
d) The change in volume with temperature
The heat capacity of an ideal gas at constant volume is given by:
a) CV = 3/2R
b) CV = 5/2R
c) CV = 7/2R
d) CV = 9/2R
The standard enthalpy of formation of a substance is defined as:
a) The enthalpy change when one mole of the substance is formed from its elements in their standard states.
b) The enthalpy change when one mole of the substance is burned completely in oxygen.
c) The enthalpy change when one mole of the substance is dissolved in water.
d) The enthalpy change when one mole of the substance is vaporized.
The third law of thermodynamics states that:
a) The entropy of a perfect crystal at absolute zero is zero.
b) The entropy of the universe is always increasing.
c) The heat flow between two objects is proportional to their temperature difference.
d) The enthalpy change of a reaction is equal to the sum of the enthalpies of formation of the products minus the sum of the enthalpies of formation of the reactants.
The enthalpy change for a reaction is -140 kJ/mol. If the reaction produces 50 g of product, what is the heat released or absorbed by the reaction?
a) -70 kJ
b) -280 kJ
c) +70 kJ
d) +280 kJ
The change in entropy of a system undergoing an isothermal process is given by:
a) ΔS = Q/T
b) ΔS = ΔU/T
c) ΔS = PΔV/T
d) ΔS = ΔH/T
Which of the following is an example of an adiabatic process?
a) A gas is compressed in a cylinder with a piston.
b) A liquid is heated in a beaker on a hot plate.
c) A metal rod is cooled in a water bath.
d) A balloon is allowed to rise in the atmosphere.
The maximum amount of work that can be obtained from a system is given by:
a) ΔU + ΔH
b) ΔU – ΔH
c) TΔS
d) -TΔS
The Joule-Thomson coefficient of an ideal gas is zero when the gas is:
a) compressed isothermally
b) expanded isothermally
c) compressed adiabatically
d) expanded adiabatically
Which of the following statements is true regarding the Gibbs free energy change (ΔG) for a chemical reaction?
a) ΔG is always positive for an exothermic reaction.
b) ΔG is always negative for an endothermic reaction.
c) ΔG is always negative for a spontaneous reaction at constant temperature and pressure.
d) ΔG is always positive for a spontaneous reaction at constant temperature and pressure.
The standard molar entropy of a substance:
a) is always positive
b) is always negative
c) can be either positive or negative
d) is always zero
The enthalpy change for the reaction 2H2(g) + O2(g) → 2H2O(l) is -571.6 kJ/mol. What is the enthalpy change for the reverse reaction?
a) +571.6 kJ/mol
b) -285.8 kJ/mol
c) -571.6 kJ/mol
d) +285.8 kJ/mol
A system undergoes a process in which the volume remains constant and the temperature increases. Which of the following statements is true regarding the internal energy (ΔU) and the heat (Q) exchanged by the system?
a) ΔU is negative and Q is positive.
b) ΔU is positive and Q is negative.
c) ΔU is positive and Q is positive.
d) ΔU is negative and Q is negative.
The entropy change of a system is given by:
a) ΔS = Q/T
b) ΔS = ΔU/T
c) ΔS = PΔV/T
d) ΔS = ΔH/T
The work done in an isothermal expansion of an ideal gas is given by:
a) W = nRTln(Vf/Vi)
b) W = -PΔV
c) W = -ΔH
d) W = -ΔU
The reversible work done in a process is:
a) always greater than the irreversible work done in the same process
b) always equal to the irreversible work done in the same process
c) always less than the irreversible work done in the same process
d) not related to the irreversible work done in the same process
The entropy change of the universe for a spontaneous process is:
a) always positive
b) always negative
c) can be either positive or negative
d) is always zero
We hope there NEET MCQ of Class 11 Thermodynamics will help you to score an excellent rank in NEET-UG. If you have any queries feel free to write in the comments section. We at Study Rate are always ready to serve our students.
